What is the molarity of hydrochloric acid in a solution that contains a $3.65g$ mass of $HCl(g)$ in $500mL$ aqueous solution?

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Answer 1 · 2017-05-09T06:33:23

$"Molarity"-="Moles of solute"/"Volume of solution"$

And here, $"molarity"=((3.65*g)/(36.5*g*mol^-1))/(500*mLxx10^-3*L*mL^-1)=0.200*mol*L^-1$ .

Is the calculation consistent dimensionally?

And thus if it is $0.200*mol*L^-1$ with respect to hydrogen chloride, it is $0.200*mol*L^-1$ with respect to $H_3O^+$ , AND $Cl^-$ .

What is the $pH$ of this solution?

What is the molarity of hydrochloric acid in a solution that contains a 3.65*g3.65*g mass of HCl(g)HCl(g) in 500*mL500*mL aqueous solution?